Calculating Molar Mass from Freezing Point Depression

This short video shows you how to calculate the molar mass of a nonelectrolyte (van't hoff=1) using freezing point depression.
Example Question:
The freezing point of a solution that contains 1.00 g of an unknown compound, dissolved in 10.0 g of benzene is found to be 2.07oC. The freezing point of pure benzene is 5.48 oC. The molal freezing point depression constant of benzene is 5.12 oC /molal. What is the molecular weight of the unknown compound?

[Lexyvil]

From all the videos I've watched online that concerns with finding an unknown substance based on the new freezing point of a solution after a mix, this one has helped me the most at finally understanding the idea behind how all the calculations relate. Thank you!

[zacht]

no joke, i've been trying to finish this lab for 2 hours and couldn't solve this question. I have to leave for class in 20 minutes but im still taking the time to type out that this video was awesome. It wasn't the same question, in fact it was almost the reverse of it. But this still helped more than any other youtube channel or chem help website. Thanks for the help!

[Lady_Katie]

Thank you so much! I have been struggling for hours on a problem like this! You're awesome :)

[ernestinasoriano]

ur such a life saver and helped me undertand my chem lab !!! AMAZING AND I MEAN AMAZING explanation

[awkwardlykylie]

THANK YOU SO MUCH. This is literally the most helpful thing ever. You are fantastic. Thank you for existing.

[benpham]

shouldn't the freezing point of solution be subtracted from freezing point of pure benzene and not the other way around?

[willambailey]

Why did the depression constant for benzene change to negative?

[tonibrat]

Thank you, you just helped me with my lab report!

[allisonmorgan]

You really know your stuff! Thank you for the video, it helped a lot.

[fishfreak]

This was everything I needed. Thanks for the helpful video!

[VQM]

Thank you for making this, helped out a lot!

[floaxclive]

YOU JUST SAVED MY ASS ^_^

Both my ass and my assignment :')
Thank you so much!!!

[carlderrick]

Is it right that freezing point depression = freezing point of solution (minus) freezing point of pure solvent?
Because some of the example that I saw, they uses freezing point of pure solvent (minus) frezzing point of solution to find the freezing point depression.

[BumbleBee]

So helpful, thanks so much! :') makes so much more sense now

[buffalobill]

Do you not have to put the kg back to g?

[lilymarayan]

help🙏🙏. About this Calculate the molar mass of sucrose in a solution prepared by dissolving 4.27 grams glucose in 50.0 grams water. The solution boils at 100.3°C which is above the normal boiling point of pure water. Kb=0.512°C/m

[TravelingYordle]

Do I need to convert to g if the given value of the mass of the unknown compound is in kg?

[TheEternalMoonlight]

Thank you so much for this.  It really helped me out a ton.  

And am I the only one who laughed when the molality was .666?  I'm sure of it now.  my chemistry teacher is satan, since it took this example to teach me how to do it.